e able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for the reactions in B1, B2, and B3 below? The following reaction will be studied: Mg(OH)2 (s) ⇌ Mg2+ (aq) + 2 OH¯ (aq) We start with MgCl2
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Le Châtelier’s Principle is described in terms of adding/removing reactants or products. While it is easy to add reactants/products, describe how we are able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for the reactions in B1, B2, and B3 below?
The following reaction will be studied:
Mg(OH)2 (s) ⇌ Mg2+ (aq) + 2 OH¯ (aq)
We start with MgCl2 solution in wells B1, B2, B3, B4, and B5.
We use phenolphthalein is an indicator that is colorless in acidic solutions and violet/pink in basic solutions.
To well B1 of MgCl2, we add 5 drops of concentrated (0.5 M) NaOH to well B1 (it turns light pink) and then we add a few drops HCl and it becomes clear.
To well B2 of MgCl2, we only add dilute NaOH until it turns pink.
To Well B3 of MgCl2, we add 1-2 drops of dilute NaOH from a dropper bottle to well B3 to get a faint pink
solution and then we add 3-5 drops EDTA and solution gets dark pink. EDTA is a ligand that reacts strongly with metal ions such as Mg2+:
Mn+ + EDTA4- ⇌ M(EDTA)n-4
Well B4 of MgCl2: We add 5 drops concentrated NaOH and heat well B4. It's light pink.
Well B5 of MgCl2: We add 5 drops concentrated NaOH and cool down B5 in a ice water bath. It gets darker pink
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